Determine the equilibrium constant for this reaction at 400 K. State and justify any assumptions or approximations that you make.
A vessel initially contains 10 moles of pure liquid A at P=5 atm and T=400 K. The following reaction occurs isothermally and isobarically until equilibrium is achieved:
A ?2B
Thermochemical data on the two compounds in the liquid phase is presented in the following table. Values of G and H were obtained with a reference pressure of 1 bar:
Apply the short-cut van`t Hoff equation to calculate the equilibrium constant @ 400K. Assume that the enthalpy change of the reaction is constant with respect to temperature. This is justified, since ?C_P?0:
Apply the short-cut van`t Hoff equation to calculate the equilibrium constant @ 400K. Assume that the enthalpy change of the reaction is constant with respect to temperature. This is justified, since ?C_P?0:
Substitute known terms into van`t Hoff equation:
Substitute ??G_400K^0 into definition of equilibrium constant:
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